Question

Assertion: If the activation energy of reaction is low, it proceeds at a faster rate.

Reason: Lowering activation energy increases the kinetic energy of molecules.

• A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion
• B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
• C. Assertion is true but Reason is false
• D. Assertion is false but Reason is true
• E. Both Assertion and Reason are false

Answer 1

The correct option is C Assertion is true but Reason is false

If activation energy of reaction is low, it proceeds at faster rate.
This is given by Arrhenius equation $k=A{e}^{-E_a/RT}$
Thus, low activation energy will result in low value of the term $E_a/RT$, high value of the term $e^{-E_a/RT}$ and high value of k.